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Question 1
This question is about the production of ammonia from nitrogen and hydrogen. |
a) | State the name of the industrial process used to manufacture ammonia.
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b) | Complete the balanced symbol equation to show the reaction between nitrogen and hydrogen to form ammonia.
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c) | State the meaning of the ⇋ symbol.
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d) | Iron is used as a catalyst in this process. Explain the purpose of the iron catalyst.
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e) | This process is completed at a temperature of 450°C. Explain why a temperature of 450°C is used.
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Question 2
This question is about the Haber process and the production of ammonia. |
a) | Which of the following would increase the percentage yield of ammonia produced in the Haber process? A increase the pressure of the reaction B decrease the pressure of the reaction C include an iron catalyst D increase the temperature of the reaction
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b) | Which of the following statements is correct when the reaction reaches equilibrium? A the reverse reaction starts to take place B the amounts of nitrogen, hydrogen and ammonia are equal C the amounts of nitrogen, hydrogen and ammonia become constant D the reaction stops
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c) | The Haber process is carried out at 200 atmospheres. Explain what effect a pressure lower than 200 atmospheres would have on:
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d) | Explain the purpose of the iron catalyst in the Haber process.
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Question 3
This question is about the industrial process of making ammonia. Ammonia is produced by reacting hydrogen with nitrogen. The equation for the reaction is below. N2 + 3H2 ⇋ 2NH3 |
a) | The production of ammonia is an exothermic reaction. Explain the effect of increasing the temperature on the percentage yield of ammonia.
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b) | State the name of the catalyst used in the Haber process.
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c) | The reaction reaches a dynamic equilibrium. What happens to the rate of the forward and backward reactions at dynamic equilibrium?
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d) | State what happens to the position of the dynamic equilibrium and the yield of ammonia when the pressure is increased. Explain why this shift occurs.
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Question 4
This question is about the Haber process. |
a) | Name the product produced by the Haber process.
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b) | Explain why the product named in part a) can be extracted when the gases pass through a condenser.
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c) | The chemical formula for the product of the Haber process is NH3. Draw a dot and cross diagram to represent a molecule of NH3.
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d) | State the type of bond found between the nitrogen and hydrogen atoms.
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Question 5
This question is about NPK fertilisers. |
a) | Some rocks contain calcium phosphate. When treated with acid they produce soluble salts, which can be used as fertilisers. Write a word equation for the reaction between calcium phosphate and nitric acid.
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b) | Fertilisers can be compared using their NPK value. One fertiliser has an NPK value of 12:11:13. Explain why this information is useful to farmers.
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c) | Ammonia is used to make fertilisers. Ammonia is formed during the Haber process. The equation for the Haber process is below. N2 + 3H2 ⇋ 2NH3 The Haber process takes place at a specific temperature and pressure. State the temperature and pressure used in the Haber process.
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d) | Describe how increasing the temperature would affect the percentage yield of ammonia.
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Question 6
Ammonium sulfate is a fertiliser manufactured from ammonia and sulfuric acid. |
a) | Sulfur is made during the contact process. The process consists of three main stages:
Write a balanced symbol equation for each stage.
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b) | The formation of sulfur trioxide in stage 2 is a reversible process. Explain how using a very high temperature affects the percentage yield of sulfur trioxide.
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c) | Explain the purpose of the vanadium oxide catalyst.
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d) | The reaction of sulfur dioxide and oxygen is normally carried out at a pressure of 1-2 atm. Explain the effect of carrying out the process at a higher pressure on the rate of attainment of equilibrium.
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